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(a)
Interpretation: The balancing of
NO3−(aq)+ Br−(aq)→NO(g) + Br2(l)
Concept Introduction: A Redox reaction leads to oxidation and reduction processes simultaneously. Oxidation and reduction reactions are the processes involved loss or gain electron. Oxidation is the process that involves the loss of electrons and oxidized to cation whereas reduction is the process that involves the gain of electrons and reduced to anion.
(a)
Answer to Problem 7RQ
2 NO3−+6 Br−+ 8 H+→2 NO + 4 H2O+ 3 Br2
Explanation of Solution
To
Step-1:
Assign oxidation number to each atom:
NO3−(aq)+ Br−(aq)→NO(g) + Br2(l) +5 -2 -1 +2-2 0
Step-2:
Write half reactions:
NO3−(aq)→NO(g) (Reduction)Br−(aq)→Br2(l) (Oxidation)
Step-3:
Balance all atoms, O with H2O and H with H+ ions:
NO3-+ 4H+→NO + 2 H2O (Reduction)2 Br-→Br2 (Oxidation)
Step-4:
Balance charges:
NO3−+ 4H+→NO + 2 H2O + 3 e- (Reduction)2 Br−→Br2 + 2 e- (Oxidation)
Step-5:
Add both equation:
NO3−+4H+→NO + 2 H2O + 3 e- (Reduction)2 Br−→Br2 + 2 e- (Oxidation)____________________________________2 NO3−+6 Br−+ 8 H+→2 NO + 4 H2O+ 3 Br2
Thus, the balance equation is:
2 NO3−+6 Br−+ 8 H+→2 NO + 4 H2O+ 3 Br2
(b)
Interpretation: The balancing of oxidation- reduction reaction by using half-reaction method in acidic medium needs to be performed.
Ni(s)+ NO3−(aq)→Ni2+(aq) + NO2(g)
Concept Introduction: A Redox reaction leads to oxidation and reduction processes simultaneously. Oxidation and reduction reactions are the processes involved loss or gain electron. Oxidation is the process that involves the loss of electrons and oxidized to cation whereas reduction is the process that involves the gain of electrons and reduced to anion.
(b)
Answer to Problem 7RQ
2 NO3−(aq)+Ni(s)+ 4 H+→Ni2+(aq) + 2 NO2(g)+ 2 H2O
Explanation of Solution
To balance the redox reaction by half-reaction or ion-electron method, add both the half-reactions by balancing the charges and atoms.
Step-1:
Assign oxidation number to each atom:
Ni(s)+ NO3−(aq)→Ni2+(aq) + NO2(g) 0 +5 -2 +2 +4-2
Step-2:
Write half reactions:
NO3−(aq)→ NO2(g) (Reduction)Ni(s)→Ni2+(aq) (Oxidation)
Step-3:
Balance all atoms, O with H2O and H with H+ ions:
NO3−(aq)+ 2 H+→ NO2(g)+ H2O (Reduction)Ni(s)→Ni2+(aq) (Oxidation)
Step-4:
Balance charges:
NO3−(aq)+ 2 H+→ NO2(g)+ H2O (Reduction)Ni(s)→Ni2+(aq)+ 2 e- (Oxidation)
Step-5:
Add both equation:
NO3−(aq)+ 2 H++e- → NO2(g)+ H2O (Reduction)Ni(s)→Ni2+(aq)+ 2 e- (Oxidation)____________________________________2 NO3−(aq)+Ni(s)+ 4 H+→Ni2+(aq) + 2 NO2(g)+ 2 H2O
Thus, the balance equation is:
2 NO3−(aq)+Ni(s)+ 4 H+→Ni2+(aq) + 2 NO2(g)+ 2 H2O
(c)
Interpretation: The balancing of oxidation- reduction reaction by using half-reaction method in acidic medium needs to be performed.
ClO4−(aq)+ Cl−(aq)→ClO−3(aq) + Cl2(g)
Concept Introduction: A Redox reaction leads to oxidation and reduction processes simultaneously. Oxidation and reduction reactions are the processes involved loss or gain electron. Oxidation is the process that involves the loss of electrons and oxidized to cation whereas reduction is the process that involves the gain of electrons and reduced to anion.
(c)
Answer to Problem 7RQ
2 Cl-(aq)+ClO4-(aq)+ 2 H+→ClO-3(aq) + ClO2(g)+ H2O
Explanation of Solution
To balance the redox reaction by half-reaction or ion-electron method, add both the half-reactions by balancing the charges and atoms.
Step-1:
Assign oxidation number to each atom:
ClO4−(aq)+ Cl−(aq)→ClO−3(aq) + Cl2(g) +7 -2 -1 +5 -2 0
Step-2:
Write half reactions:
ClO4−(aq)→ClO−3(aq) + Cl2(g) (Reduction)Cl−(aq)→ClO−3(aq) + Cl2(g) (Oxidation)
Step-3:
Balance all atoms, O with H2O and H with H+ ions:
3 Cl-(aq)+3H2O→ClO-3(aq) + Cl2(g)+ 6 H+ (Oxidation)ClO4-(aq)+ 18 H+ →ClO-3(aq) + Cl2(g)+9 H2O (Reduction)
Step-4:
Balance charges:
3 Cl-(aq)+3H2O→ClO-3(aq) + Cl2(g)+ 6 H+ + 8 e- (Oxidation)ClO4-(aq)+ 18 H++ 16 e- →ClO-3(aq) + Cl2(g)+9 H2O (Reduction)
Step-5:
Add both equation:
3 Cl-(aq)+ 3H2O→ClO-3(aq) + Cl2(g)+ 6 H+ + 8 e- (Oxidation)ClO4-(aq)+ 18 H++ 16 e- →ClO-3(aq) + Cl2(g)+9 H2O (Reduction)_____________________________________________________2 Cl-(aq)+ClO4-(aq)+ 2 H+→ClO-3(aq) + ClO2(g)+ H2O
Thus, the balance equation is:
2 Cl-(aq)+ClO4-(aq)+ 2 H+→ClO-3(aq) + ClO2(g)+ H2O
Chapter 18 Solutions
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